CHM 1046 Quiz 1

Which one of the following correctly ranks the compounds in order of lowest vapor pressure to highest vapor pressure based only in intermolecular forces? A) CH₃CH₂OH < CH₃OCH₃ < CH₃CH₂CH₃ B) CH₃OCH₃ < CH₃CH₂CH₃ < CH₃CH₂OH C) CH₃CH₂CH₃ < CH₃CH₂OH < CH₃OCH₃ D) CH₃CH₂CH₃ < CH₃OCH₃ < CH₃CH₂OH

A) CH₃CH₂OH < CH₃OCH₃ < CH₃CH₂CH₃

Which one of the following would have the largest dispersion forces? A) CH₃CH₂SH B) CH₃NH₂ C) CH₄ D) CH₃CH₃

A) CH₃CH₂SH

Which one of the following would have the highest heat of vaporization? A) CH₃OH B) CH₂F₂ C) NF₃ D) CHF₃

A) CH₃OH

Which of the following has the lowest boiling point? A) C₅H₁₂ B) C₇H₁₆ C) C₉H₂₀ D) C₁₁H₂₄ E) C₁₃H₂₈

A) C₅H₁₂

Which of the following should exhibit the highest viscosity at 298 K? A) HOCH₂CH₂OH B) CH₃OCH₃ C) CH₃OH D) CH₃Br E) CH₂Cl₂

A) HOCH₂CH₂OH

Dispersion forces would be weakest in which of the following substances? A) He B) Ne C) Ar D) Kr E) Xe

A) He

Which of the following would you expect to have the lowest boiling point? A) H₂ B) F₂ C) HF D) H₂S

A) H₂

Which combination of properties would be expected to lead to the most viscous liquid? A) Strong intermolecular forces, low temperature B) Strong intermolecular forces, high temperature C) Weak intermolecular forces, low temperature D) Weak intermolecular forces, high temperature.

A) Strong intermolecular forces, low temperature

What intermolecular forces are present between two molecules of CF₃CF₃? A) dispersion only B) dipole-dipole only C) dispersion and dipole-dipole D) dispersion and hydrogen bonding E) dipole-dipole and hydrogen bonding

A) dispersion only

Which of the following represents the intermolecular forces present in CO₂? A) dispersion only B) dipole-dipole only C) hydrogen bonding only D) dispersion and dipole-dipole E) dispersion and hydrogen bonding

A) dispersion only

Which best explains why the trend in noble gas boiling points increases down the group? A) increasing dispersion interactions B) increasing dipole-dipole interactions C) increasing ion-dipole interactions D) increasing hydrogen bonding interactions E) increasing ion-ion interactions

A) increasing dispersion interactions

Which of the following pairs of substances has the higher vapor pressure at 298 K given first? A) H₂O, H₂Se B) CF₄, CBr₄ C) Kr, Ne D) C₆H₁₄, C₄H₁₀ E) CH₃OH, CH₃OCH₃

B) CF₄, CBr₄

Which of the following substances is a liquid at room temperature? A) CH₃CH₃ B) CH₃OH C) CH₄ D) HCl E) CF₄

B) CH₃OH

Which of the following substances is not a gas at 298 K and 1 atm? A) CO₂ B) CH₃OH C) C₂H₆ D) O₂ E) C₃H₈

B) CH₃OH

Which of the following is predicted to have the lowest boiling point? A) I₂ B) CS₂ C) CCl₄ D) CBr₄ E) SF₆

B) CS₂

Which of the following pairs correctly ranks the viscosity of the compounds? A) H₂O < CCl₄ B) C₅H₁₂ < C₆H₁₄ C) C₂H₅OH < C₂H₆ D) C₈H₁₈ < C₂H₆

B) C₅H₁₂ < C₆H₁₄

Which of the following would you expect to have the highest boiling point? A) H₂ B) NH₃ C) N₂ D) CH₄

B) NH₃

Which best explains why the meniscus of mercury in a glass tube is convex? A) The greater attraction of mercury to the glass than to itself. B) The lower attraction of mercury to the glass than to itself. C) The low surface tension of mercury. D) The high density of mercury compared to water. E) The repulsion between mercury and the glass.

B) The lower attraction of mercury to the glass than to itself.

What intermolecular forces are present between two molecules of CH₃CF₃? A) dispersion only B) dispersion and dipole-dipole C) dispersion, dipole-dipole, and hydrogen bonding D) dispersion and hydrogen bonding

B) dispersion and dipole-dipole

Which one of the following correctly ranks the compounds in order of lowest enthalpy of vaporization to highest enthalpy of vaporization based only in intermolecular forces? A) CH₃NH₂ < CH₃SH < CH₃CH₃ B) CH₃NH₂ < CH₃CH₃ < CH₃SH C) CH₃CH₃ < CH₃SH < CH₃NH₂ D) CH₃SH < CH₃NH₂ < CH₃CH₃

C) CH₃CH₃ < CH₃SH < CH₃NH₂

Which of the following bonds is a polar covalent bond? A) Li - Cl B) Cl - Cl C) H - Cl D) Li - Li

C) H - Cl

Rank the following compounds in order of lowest boiling point to highest boiling point based on intermolecular forces. A) HF < HCl < HBr < HI B) HI < HBr < HCl < HF C) HCl < HBr < HI < HF D) HBr < HI < HF < HCl

C) HCl < HBr < HI < HF

Which of the following substances would not exhibit any hydrogen bonding interactions in a pure substance? A) H₂O B) HF C) N(CH₃)₃ D) CH₃CH₂OH E) CH₃NH₂

C) N(CH₃)₃

Which of the following exhibits dipole-dipole intermolecular forces? A) BF₃ B) CO₂ C) NH₃ D) Br₂ E) CF₄

C) NH₃

When the temperature of a liquid increases what happens to the viscosity and surface tension of the liquid? A) Viscosity increases, surface tension increases. B) Viscosity increases, surface tension decreases. C) Viscosity decreases, surface tension decreases. D) Viscosity decreases, surface tension increases.

C) Viscosity decreases, surface tension decreases.

Which of the factors contributes to a low viscosity of a liquid? A) high boiling point B) hydrogen bonding C) compact molecular shape D) low temperature E) high molar mass

C) compact molecular shape

What intermolecular forces are present between two molecules of CH₃OCH₂CH₃? A) dispersion only B) dipole-dipole only C) dispersion and dipole-dipole D) dispersion and hydrogen bonding E) dipole-dipole and hydrogen bonding

C) dispersion and dipole-dipole

Ammonia and hydrogen fluoride both have unusually high boiling points due to _____ A) dispersion forces. B) dipole-dipole interactions. C) hydrogen bonding. D) ion-dipole interactions. E) low molar masses.

C) hydrogen bonding.

The intermolecular force found in Na⁺(aq) is _____ A) ionic bonds. B) dipole-dipole interactions. C) ion-dipole interactions. D) dispersion forces. E) covalent bonds.

C) ion-dipole interactions.

Which property typically indicates strong intermolecular forces are present in a liquid? A) low heat of vaporization B) low critical temperature C) low vapor pressure D) low boiling point E) low melting point

C) low vapor pressure

Which one of the following correctly ranks the compounds in order of lowest boiling point to highest boiling point based only in intermolecular forces? A) CH₃CH₂OH < CH₃OCH₃ < CH₃CH₃CH₃ B) CH₃OCH₃ < CH₃CH₂CH₃ < CH₃CH₂OH C) CH₃CH₂CH₃ < CH₃CH₂OH < CH₃OCH₃ D) CH₃CH₂CH₃ < CH₃OCH₃ < CH₃CH₂OH

D) CH₃CH₂CH₃ < CH₃OCH₃ < CH₃CH₂OH

Which of the following would exhibit hydrogen bonding? A) HCl B) CH₃CH₃ C) CF₂H₂ D) CH₃CH₂OH E) CH₃OCH₃

D) CH₃CH₂OH

Which of the following bonds is a nonpolar covalent bond? A) H - F B) N - F C) F - Cl D) F - F

D) F - F

Which of the following has the lowest freezing point? A) H₂O B) N₂ C) SO₂ D) H₂ E) CO₂

D) H₂

Which of the following halogens would have the highest boiling point? A) F₂ B) Cl₂ C) Br₂ D) I₂

D) I₂

Which of the following halogens would have the highest melting point? A) F₂ B) Cl₂ C) Br₂ D) I₂

D) I₂

What intermolecular forces are present between two molecules of CH₃CH₂SH? A) dispersion only B) dipole-dipole only C) hydrogen bonding only D) dispersion and dipole-dipole E) dispersion and hydrogen bonding

D) dispersion and dipole-dipole

What intermolecular forces are present between two molecules of HI? A) dispersion only B) dipole-dipole only C) hydrogen bonding only D) dispersion and dipole-dipole E) dispersion and hydrogen bonding

D) dispersion and dipole-dipole

The intermolecular force between molecules of I₂ is _____ A) ionic bonds. B) dipole-dipole interactions. C) ion-dipole interactions. D) dispersion forces. E) covalent bonds.

D) dispersion forces.

Which of the following straight-chain hydrocarbons will have the highest viscosity at 298 K? A) C₅H₁₂ B) C₆H₁₄ C) C₇H₁₆ D) C₈H₁₈ E) C₉H₂₀

E) C₉H₂₀

Which is expected to have the highest heat of vaporization? A) CH₄ B) SiH₄ C) NH₃ D) PH₃ E) H₂O

E) H₂O

Which is expected to have the lowest vapor pressure? A) CH₄ B) SiH₄ C) NH₃ D) PH₃ E) H₂O

E) H₂O

Which of the following substances would have the greatest dispersion forces? A. H2 B. O2 C. Cl2 D. Br2 E. I2

I2

when IMF increases what happens to viscosity

IMF increases, viscosity increases

van der waals

IMF of attraction between neutral molecules, dipole-dipole, London dispersion, hydrogen bonding

What are the IMFS in Ne

London

What are the IMFS in CH3Cl

London, dipole-dipole

What are the IMFS in CO

London, dipole-dipole

What are the IMFS in HCl

London, dipole-dipole

What are the IMFS in CH3OH

London, dipole-dipole, hydrogen bond

What are the IMFS in HF

London, dipole-dipole, hydrogen bond

What are the IMFS in NH3

London, dipole-dipole, hydrogen bond

dipole-induced dipole

a polar molecule interacting with a nonpolar one

Chlorine has a critical temperature of 144°C and a critical pressure of 77 atm. Under which of the following conditions would Cl2 most likely be a liquid? a) 125°C, 70 atm b) 125°C, 30 atm c) 150°C, 70 atm d) 150°C, 30 atm

a) 125°C, 70 atm

Rank the following liquids in order of increasing boiling points, from lowest to highest: He / NH3 / Ar / N2 a) He < N2 < Ar < NH3 b) He < Ar < N2 < NH3 c) NH3 < Ar < N2 < He d) NH3 < N2 < Ar < He

a) He < N2 < Ar < NH3

Which of the following pure substances exhibits hydrogen bonding? a) NH3 b) H2S c) HCl d) CH4 e) all of these do

a) NH3

what is an example of dipole-dipole?

acetone with acetone, triethyl amine with acetone

Which is the weakest intermolecular force among a group of molecules of comparable molecular weight (molar mass)? a) dipole-dipole b) London c) ionic bonding d) hydrogen bonding

b) London

The interaction responsible for the cohesive intermolecular forces of liquid nitrogen is: a) hydrogen bonding b) the London dispersion force c) dipole-dipole interaction d) covalent bonding

b) the London dispersion force

Arrange these substances in order of INCREASING boiling point: Xe, H2, H2O, LiCl, H2S. a) Xe < H2 < H2O < LiCl < H2S b) Xe < H2 < H2S < H2O < LiCl c) H2 < Xe < H2S < H2O < LiCl d) H2 < Xe < H2O < H2S < LiCl

c) H2 < Xe < H2S < H2O < LiCl

Which of the following substances will have the highest boiling point? a) methane (MW=16) b) butane (MW=58) c) ethyl alcohol (MW=46) d) methyl alcohol (MW=32)

c) ethyl alcohol (MW=46)

The intermolecular forces that are most significant in accounting for the high boiling point of liquid water relative to other substances of similar molecular weight are the: a) ion-ion attractions b) London dispersion forces c) hydrogen bonding forces d) dipole-dipole attractions

c) hydrogen bonding forces

what is an example of dipole-induced dipole?

carbon dioxide in water, carbon dioxide in ethylene

Based on Coulomb's law of interaction strength between ions, which of the following compounds has the highest melting point? a) CaCl2 b) NaCl c) NaF d) MgO

d) MgO

Which of the following substances will have the lowest boiling point? a) neon b) water c) ammonia d) helium

d) helium

increase in vapor pressure == _________ IMF

decrease

hydrogen bonding

dipole-dipole when H is bonded to N, O, F

what is an example of ion-dipole force

dissolving any ionic compound in water

Which response lists interparticle forces (between molecules of comparable size) in order of increasing strength? a) London < ionic < H-bonds < dipole b) dipole < London < H-bond < ionic c) H-bond < ionic < dipole < London d) ionic < H-bond < London < dipole e) London < dipole < H-bond < ionic

e) London < dipole < H-bond < ionic

larger the dipole, _______ melting point and ______ boiling point

higher melting point and higher boiling point

London dispersion

holds together non polar molecules together

ion-dipole

interaction of ion (cation + anion) with polar molecule

dipole-dipole

interaction of polar molecules between other polar molecules

Rank the IMFS from strongest to weakest

ionic bonds> ion-dipole> Hydrogen bonding> dipole-dipole>> London dispersion

What are the IMFS in C2H4

london

What are the IMFS in CO2

london

London dispersion forces have _______ melting points, and _______ boiling points

low melting and boiling points

ionic forces

result of electrostatic forces between ions

when do London dispersion forces increase?

when strength and molecular weight increases